PERCENT YIELD tells you the efficiency of a reaction tells you the efficiency of a reaction formula: formula: % yield = actual yield x 100 theoretical.

Slides:

Advertisements

Similar presentations

Stoichiometry Continued…

Advertisements

II. Stoichiometry in the Real World (p ) Stoichiometry – Ch. 9.

Chapter 5 Chemical Reactions

Limiting Reactants and Percent Yield

II. Stoichiometry in the Real World Limiting Reagents and % yield (p ) Stoichiometry – Ch. 12.

Chapter 9 - Section 3 Suggested Reading: Pages

Copyright © Houghton Mifflin Company. All rights reserved. 9 | 1 Information Given by the Chemical Equation Balanced equations show the relationship between.

Lecturer: Amal Abu- Mostafa.  Available Ingredients ◦ 4 slices of bread ◦ 1 jar of peanut butter ◦ 1/2 jar of jelly Limiting Reactant Limiting Reactant.

Chapter 9 Chemical Quantities. 9 | 2 Information Given by the Chemical Equation Balanced equations show the relationship between the relative numbers.

Limiting/Excess Reactants and Percent Yield

Limiting Reactants and Percent Yields

UNIT VII Excess & Percentage Yield Unit 7: Lesson 2.

Chapter 9 – Review Stoichiometry

Limiting and Excess Reagents

Limiting Reagent u The limiting reagent is the reactant you run out of first. u The excess reagent is the one you have left over. u The limiting reagent.

Limiting Reagents and Percent Yield

Identify the limiting reactant and calculate the mass of a product, given the reaction equation and reactant data. Include: theoretical yield, experimental.

Chemistry 11 Stoichiometry Reality II: Percent Yield.

Ch. 9: Calculations from Chemical Equations

Unit 8: Percent Yield Calculations

Daily Science feb How many grams of CH4 is needed to produce 50.0 g CHCl3? CH4 + 3Cl2  CHCl3 +3HCl Lithium reacts spontaneously with bromine to produce.

*Notice, kind of like the opposite of Percent Error.

 All stoichiometry problems start with a balanced equation.  You must check for this!  If it is not balanced, BALANCE IT!

Stoichiometry and the Math of Equations Part 4: Percent Yield 1.

Theoretical, Actual, and Percent Yield Problems Example 1.

Ch. 11: Stoichiometry Sec. 11.4: Percent Yield.

UNIT VII Percentage Yield. VII.5 PERCENTAGE YIELD AND PERCENTAGE PURITY: Percentage Yield : is used to describe the amount of product actually obtained.

C. Johannesson II. Stoichiometry in the Real World (p ) Stoichiometry – Ch. 9.

II. Limiting Reactants Stoichiometry – 3.7. A. Limiting Reactants b Available Ingredients 4 slices of bread 1 jar of peanut butter 1/2 jar of jelly b.

II. Stoichiometry in the Real World Stoichiometry – Ch. 11.

Chapter 9 Chemical Quantities. Copyright © Houghton Mifflin Company. All rights reserved. 9 | 2 Information Given by the Chemical Equation Balanced equations.

II. Stoichiometry in the Real World Stoichiometry.

Theoretical yield: amounts of product calculated from the limiting reagent. Actual yield: amount produced during the conducted experiment. Percentage.

1 Chapter 4 Chemical Equations and Stoichiometry.

Chapter 9, section 3, part 2 Percent Yield. Why percent yield?  Usually, not all the product possible is actually formed.  theoretical yield  maximum.

Actual and Percent Yields So far when we have been talking about reactions we have been talking about 100% of the (limiting) reactant becoming a product.

Reaction Yield. Theoretical vs Actual Yield Theoretical yield is the maximum amount of product that can be produced from a given amount of reactant Calculated.

Percentage Yield.

Percent Yield How efficient is a chemical reaction?

GOOD AFTERNOON! Prepare to take notes. You will be allowed to use these notes on the test next week! You will need: 1.Something to write on 2.Something.

Section 9.3 Limiting Reactants and Percent Yield 1.Define the terms theoretical yield and actual yield. 2.Calculate percent yield 3.Identify reasons that.

1 Percent Yield. 2 Theoretical, Actual, and Percent Yield Theoretical yield The maximum amount of product calculated using the balanced equation. Actual.

WARM UP 1.Given the following reaction…… Ba(NO 3 ) 2(aq) + Na 2 CO 3(aq)  BaCO 3(s) + 2 NaNO 3(aq) Calculate the yield of sodium nitrate when you start.

Ch. 9-3 Limiting Reactants & Percent Yield. POINT > Define limiting reactant POINT > Identify which reactant is limiting in a reaction POINT > Define.

SOL Review 6 Stoichiometry. Consider: 4NH 3 + 5O 2  6H 2 O + 4NO Many conversion factors exist: 4 NH 3 6 H 2 04NO 5O 2 (and others) 5 O 2 4 NO4 NH 3.

Challenge Problem When nitrogen and hydrogen react, they form ammonia gas, which has the formula NH 3. If 56.0 g of nitrogen are used up in the reaction,

Mass-Mass Conversions 56.0 g N 2 x g N 2 g NH = 1904 = When nitrogen and hydrogen react, they form ammonia gas, which has the formula.

Stoichiometry – Ch What would be produced if two pieces of bread and a slice of salami reacted together? + ?

THIS IS With Host... Your VocabularyMole to mole Limiting Reactants Mass to mass Mass to Mole Percent Yield.

UNIT VII Excess & Percentage Yield Unit 7: Lesson 2.

Stoichiometry in the Real World Stoichiometry – Ch. 11.

II. Stoichiometry in the Real World (p )

Percent Yield actual yield % yield = x 100 theoretical yield

II. Stoichiometry in the Real World

Percentage Yield.

Ch. 9: Calculations from Chemical Equations

Theoretical Yield The maximum amount of product that can be produced from a given amount of reactant.

Agenda: 1/13/2017 Go over the procedure for the Molarity Lab

Stoichiometry in the Real World

II. Stoichiometry in the Real World (p )

*Notice, kind of like the opposite of Percent Error.

II. Stoichiometry in the Real World (p )

Lecture 4.5 – Percent Yield

II. Stoichiometry in the Real World

Bellwork Tuesday 5.9 L of carbon dioxide is combined with 8.4 g MgO in a synthesis reaction to form magnesium carbonate. How many grams of magnesium carbonate.

Percentage Yield.

Limiting/Excess Reactants and Percent Yield

Presentation transcript:

PERCENT YIELD tells you the efficiency of a reaction tells you the efficiency of a reaction formula: formula: % yield = actual yield x 100 theoretical yield theoretical yield

PERCENT YIELD theoretical yield – amt of prod predicted to form based on balanced equation theoretical yield – amt of prod predicted to form based on balanced equation actual yield – actual yield – obtained by doing an experiment obtained by doing an experiment varies according to temp, pressure, purity of reactants, and side rxns varies according to temp, pressure, purity of reactants, and side rxns

CALCULATE % YIELD Potassium carbonate reacts with HCl: write the balanced equation. K 2 CO 3(aq) + 2HCl (aq) → 2KCl (aq) + H 2 O + CO 2(g) When 45.8 g of K 2 CO 3 is added to an excess of HCl, 46.3 g KCl is recovered. Calc. % yield.

CALCULATE % YIELD K 2 CO 3(aq) + 2HCl (aq) → 2KCl (aq) + H 2 O + CO 2(g) 45.8g K 2 CO 3 x 1 mol K 2 CO 3 x 2 mol KCl … g K 2 CO 3 1 mol K 2 CO 3 x 74.55g KCl = 49.4 g KCl 1 mol KCl %yield = (46.3 g / 49.4 g) x 100 = 93.7%